Q: Which equation correctly represents the ion product constant for water ($$K_w) at$$ $$25^\circC$$?

$$K_w = [\mathrm{H^+}][\mathrm{OH^-}] = 1.0 \times 10$$^{-14}$$

Q: If the $$[\mathrm{OH^-}] in a $$solution is $$5.0 \times 10$$^{-8}$$\ \mathrm{M}$$, what is the $$[\mathrm{H_3O^+}]$$?

$$2.0 \times 10$$^{-7}$$\ \mathrm{M}$$

Q: A solution has a pH of $$2.15. $$What is the $$[\mathrm{H_3O^+}]$$?

$$7.1 \times 10$$^{-3}$$\ \mathrm{M}$$

Question 1

Which of the following statements best describes why water (H2O) is considered amphoteric?

Accepted Answer

It can donate a proton (H+) in some reactions and accept a proton (H+) in others.

Question 2

Given the reaction: $$\mathrm{NH_3$(g) + H_2O(l) \rightarrow NH_4$^+(aq) + OH^-(aq)}$$, which species is the conjugate acid of ammonia?

Accepted Answer

$$\mathrm{NH_4$^+}$$

Question 3

Which of the following acids is classified as a strong acid?

Accepted Answer

Hydrochloric acid ($$\mathrm{HCl})$$

Question 4

What is the pH of a solution with $$[\mathrm{H_3O^+}] = 1.0 	imes 10$$^{-3}$$\ \mathrm{M}$$?

Accepted Answer

$$3.00$$

Question 5

A buffer solution is made from acetic acid ($$\mathrm{HC_2H_3O_2}) $$and sodium acetate ($$\mathrm{NaC_2H_3O_2}). $$What happens when a small amount of $$\mathrm{OH^-} is $$added?

Accepted Answer

The acetic acid neutralizes the added $$\mathrm{OH^-}$$, forming more acetate ion.

Question 6

Which equation correctly represents the ion product constant for water ($$K_w) at$$ $$25^\circC$$?

Accepted Answer

$$K_w = [\mathrm{H^+}][\mathrm{OH^-}] = 1.0 	imes 10$$^{-14}$$

Question 7

If the $$[\mathrm{OH^-}] in a $$solution is $$5.0 	imes 10$$^{-8}$$\ \mathrm{M}$$, what is the $$[\mathrm{H_3O^+}]$$?

Accepted Answer

$$2.0 	imes 10$$^{-7}$$\ \mathrm{M}$$

Question 8

Which of the following best describes the effect of adding a catalyst to a reaction at equilibrium?

Accepted Answer

It increases the rate of both the forward and reverse reactions but does not change the equilibrium position.

Question 9

A solution has a pH of $$2.15. $$What is the $$[\mathrm{H_3O^+}]$$?

Accepted Answer

$$7.1 	imes 10$$^{-3}$$\ \mathrm{M}$$

Question 10

Which of the following is a correct balanced equation for the neutralization of magnesium hydroxide and nitric acid?

Accepted Answer

$$\mathrm{Mg(OH)_2(aq) + 2HNO_3(aq) \rightarrow Mg(NO_3$)_2(aq) + 2H_2O(l)}$$

Question 11

During a titration, what is the equivalence point?

Accepted Answer

The point at which the amount of titrant added is stoichiometrically equal to the number of moles of substance present in the sample.

Question 12

Which of the following statements about strong acids and their conjugate bases is correct?

Accepted Answer

Strong acids have weak conjugate bases.

Question 13

If a system at equilibrium is subjected to an increase in the concentration of a product, according to Le Chatelier’s Principle, what will happen?

Accepted Answer

The equilibrium will shift toward the reactants.

Question 14

Which of the following is a characteristic of a buffer solution?

Accepted Answer

It resists changes in pH when small amounts of acid or base are added.

Question 15

What is the molarity of an HCl solution if $$18.5\ \mathrm{mL} of$$ $$0.225\ \mathrm{M}$$ NaOH are required to neutralize $$10.0\ \mathrm{mL}$$ HCl?

Accepted Answer

$$0.416\ \mathrm{M}$$

Question 16

Which of the following substances is a strong base?

Accepted Answer

Potassium hydroxide ($$\mathrm{KOH})$$

Question 17

Which of the following best describes the relationship between $$[\mathrm{H_3O^+}]$$ and $$[\mathrm{OH^-}] in a $$neutral solution at $$25^\circC$$?

Accepted Answer

$$[\mathrm{H_3O^+}] = [\mathrm{OH^-}] = 1.0 	imes 10$$^{-7}$$\ \mathrm{M}$$

Question 18

Which of the following is a correct statement about the pH scale?

Accepted Answer

A pH less than 7 is acidic, a pH of 7 is neutral, and a pH greater than 7 is basic.

Acids, Bases, and Equilibrium: Comprehensive Study Notes for Chapter 10

Study Guide - Practice Questions

Study Guide - Flashcards